Question

calculate the wavelength of the spectral line when the electron in the hydrogen atom undergoes a transition from 4th energy level to 2nd energy level​

Answer 1

I hope this is the answer that you need

Answer 2

The wavelength of spectral line is 486.2 nm

Explanation:

To calculate the wavelength of light, we use Rydberg's Equation:

$\frac{1}{\lambda}=R_H\left(\frac{1}{n_f^2}-\frac{1}{n_i^2} \right )$

Where,

$\lambda$ = Wavelength of radiation

$R_H$ = Rydberg's Constant  = $1.097\times 10^7m^{-1}$

$n_f$ = Final energy level = 2

$n_i$ = Initial energy level = 4

Putting the values in above equation, we get:

$\frac{1}{\lambda }=1.097\times 10^7m^{-1}\left(\frac{1}{2^2}-\frac{1}{4^2} \right )\\\\\lambda =\frac{1}{2.056\times 10^6m^{-1}}=4.862\times 10^{-7}m$

Converting this into nanometers, we use the conversion factor:

$1m=10^9nm$

So, $4.862\times 10^{-7}m\times (\frac{10^9nm}{1m})=486.2nm$

Learn more about Rydberg's equation:

https://brainly.com/question/13033646

https://brainly.com/question/14545347

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